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[1] A group of Aggie students prepared vinegar in the lab by using an initial concentration of Acetic acid of 0.25M. The dissociation of the acetic acid is shown below. If the Ka of the acetic acid was 4.8 x10*,calculate the equilibrium concentration of [CH3COOH],[H3O*], [CH3COO`], pH and [OH] of the vinegar. Use The Approximation Rule if Possible CH₂COOH(aq) + H₂O(1): CH3COO +H;O* (aq) (aq)

[1] A group of Aggie students prepared vinegar in the lab by using an initial concentration of Acetic acid of 0.25M. The dissociation of the acetic acid is shown below. If the Ka of the acetic acid was 4.8 x10*,calculate the equilibrium concentration of [CH3COOH],[H3O*], [CH3COO`], pH and [OH] of the vinegar. Use The Approximation Rule if Possible CH₂COOH(aq) + H₂O(1): CH3COO +H;O* (aq) (aq)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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[1] A group of Aggie students prepared vinegar in the lab by using an initial concentration of Acetic acid of 0.25M. The dissociation of the acetic acid is shown below. If the Ka of the acetic -4 acid was 4.8 x10,calculate the equilibrium concentration of [CH3COOH],[H3O*], [CH3COO"], pH and [OH"] of the vinegar. Use The Approximation Rule if possible CH3COOH(aq) + H₂O(1) + CH3COO (aq) + H30* (aq)
Transcribed Image Text:[1] A group of Aggie students prepared vinegar in the lab by using an initial concentration of Acetic acid of 0.25M. The dissociation of the acetic acid is shown below. If the Ka of the acetic -4 acid was 4.8 x10,calculate the equilibrium concentration of [CH3COOH],[H3O*], [CH3COO"], pH and [OH"] of the vinegar. Use The Approximation Rule if possible CH3COOH(aq) + H₂O(1) + CH3COO (aq) + H30* (aq)
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